Answer: Thus the standard potential for an electrochemical cell with the cell reaction that follows is 0.84 V.
Explanation:
Standard potential for an electrochemical cell is given by:
\(E^0{cell}\) = standard electrode potential =\(E^0{cathode}-E^0{anode}\)
The \(E^0\) values have to be reduction potentials.
Given: Reduction potential for atom X:
\(E^o_{X^{2+}/X}=+0.51V\)
\(E^o_{A^{2+}/A}=-0.33V\)
The element A with negative reduction potential will lose electrons undergo oxidation and thus act as anode.The element X with positive reduction potential will gain electrons undergo reduction and thus acts as cathode.
\(X^{2+}+A\rightarrow X+A^{2+}\)
\(E^0{cell}\) = standard electrode potential =\(E^0{cathode}-E^0{anode}=+0.51-(-0.33)=0.84V\)
Thus the standard potential for an electrochemical cell with the cell reaction that follows is 0.84 V.
